`[OH^(-)]` in a solution is `1 mol L^(-1)`. The `pH` of the solution is

Options

A. `1`
B. `0`
C. `14`
D. `10^(-14)`

Explanation

To find the pH of a solution where the concentration of hydroxide ions \([OH^-]\) is \(1 \, \text{mol L}^{-1}\), we can follow these steps:

### Step 1: Calculate pOH
The pOH of a solution can be calculated using the formula:
\[ \text{pOH} = -\log[OH^-] \]
Given that \([OH^-] = 1 \, \text{mol L}^{-1}\):
\[ \text{pOH} = -\log(1) \]
Since the logarithm of 1 is 0:
\[ \text{pOH} = 0 \]

### Step 2: Use the relationship between pH and pOH
At 25°C, the relationship between pH and pOH is given by:
\[ \text{pH} + \text{pOH} = 14 \]
Substituting the value of pOH we calculated:
\[ \text{pH} + 0 = 14 \]

### Step 3: Solve for pH
Now, we can solve for pH:
\[ \text{pH} = 14 - 0 \]
\[ \text{pH} = 14 \]

### Final Answer
The pH of the solution is \(14\).

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